Thermodynamics is the branch of physical chemistry that deals with energy transfer and its relation to chemical reactions.

The rate of a chemical reaction is influenced by temperature, concentration, and activation energy.

Activation energy is the minimum amount of energy required for a chemical reaction to occur.

The second law of thermodynamics states that the total entropy of an isolated system always increases over time.

The equilibrium constant (K) is defined as the ratio of products to reactants at equilibrium.

The van der Waals equation of state takes into account intermolecular forces, ideal gas behavior, and non-ideal gas behavior.

The Arrhenius equation relates rate constant, temperature, and activation energy.

The uncertainty principle states that the more precisely the position of a particle is known, the less precisely its momentum can be known, and vice versa.

The Pauli exclusion principle states that no two electrons in an atom can have the same set of quantum numbers, which includes spin, energy, and orbital.

The Schrödinger equation is a wave equation that describes the behavior of electrons in atoms, molecules, and chemical reactions.

The Born-Oppenheimer approximation assumes that the motion of electrons and nuclei can be separated, allowing for the independent treatment of electronic and nuclear motion.

The Hartree-Fock method is a self-consistent field method that approximates the wave function of a many-electron system as a product of one-electron wave functions.

Density functional theory (DFT) is a method for calculating the electronic structure of atoms, molecules, and solids based on the electron density.

Molecular orbital theory describes the behavior of electrons in molecules, the formation of chemical bonds, and the properties of molecules.

Valence bond theory describes the formation of chemical bonds, the hybridization of atomic orbitals, and the properties of molecules.